anderson

2008 AND Prelim Chem Paper 1 1 Setter: Ms Mok Lai Koin

ANDERSON SECONDARY SCHOOL

PRELIMINARY EXAMINATION 2008

Secondary Four Express

Chemistry (SPA) (Rev) 5072/01

Paper 1 Multiple Choice

Monday 08 Sept 2008 1 hr

READ THESE INSTRUCTIONS FIRST

Write your register number and name on all the work you hand in.

Write in dark blue or black pen.

You may use a soft pencil for any diagrams, graphs or rough working

Do not use staples, paper clips, highlighters, glue or correction fluid.

There are forty questions on this paper. Answer all questions.

For each question there are four possible answers A, B, C, and D.

Choose the one you consider correct and record your choice in soft pencil on the separate

answer sheet.

Read the instructions on the answer sheet very carefully.

Each correct answer will score one mark.

A mark will not be deducted for a wrong answer. Any rough working should be done in this

booklet.

This question paper consists of 15 printed pages, including the cover page and Periodic Table.

Name: Register number ( ) Class:

The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.)

Group

I II III IV V VI VII 0

1 H

Hydrogen

1

4

He Helium

2 7

Li Lithium

3

9

Be Beryllium

4

11

B Boron

5

12

C Carbon

6

14

N Nitrogen

7

16

O Oxygen

8

19

F Fluorine

9

20

Ne Neon

10 23

Na Sodium

11

24

Mg Magnesium

12

27

Al Aluminium

13

28

Si Silicon

14

31

P Phosphorus

15

32

S Sulphur

16

35.5

Cl Chlorine

17

40

Ar Argon

18 39

K Potassium

19

40

Ca Calcium

20

45

Sc Scandium

21

48

Ti Titanium

22

51

V Vanadium

23

52

Cr Chromium

24

55

Mn Manganese

25

56

Fe Iron

26

59

Co Cobalt

27

59

Ni Nickel

28

64

Cu Copper

29

65

Zn Zinc

30

70

Ga Gallium

31

73

Ge Germanium

32

75

As Arsenic

33

79

Se Selenium

34

80

Br Bromine

35

84

Kr Krypton

36

85

Rb Rubidium

37

88

Sr Strontium

38

89

Y Yttrium

39

91

Zr Zirconium

40

93

Nb Niobium

41

96

Mo Molybdenum

42

Tc Technetium

43

101

Ru Ruthenium

44

103

Rh Rhodium

45

106

Pd Palladium

46

108

Ag Silver

47

112

Cd Cadmium

48

115

In Indium

49

119

Sn Tin

50

122

Sb Antimony

51

128

Te Tellurium

52

127

I Iodine

53

131

Xe Xenon

54 133

Cs Caesium

55

137

Ba Barium

56

139

La Lanthanium

57

178

Hf Hafnium

72

181

Ta Tantalum

73

184

W Tungsten

74

186

Re Rhenium

75

190

Os Osmium

76

192

Ir Iridium

77

195

Pt Platinum

78

197

Au Gold

79

201

Hg Mercury

80

204

Tl Thallium

81

207

Pb Lead

82

209

Bi Bismuth

83

Po Polonium

84

At Astatine

85

Rn Radon

86

Fr Francium

87

226

Ra Radium

88

227

Ac Actinium

89 +

*58-71 Lanthanoid series

+90-103 Actinoid series

140

Ce Cerium

58

141

Pr Praseodymium

59

144

Nd Neodymium

60

Pm Promethium

61

150

Sm Samarium

62

152

Eu Europium

63

157

Gd Gadolinium

64

159

Tb Terbium

65

162

Dy Dysprosium

66

165

Ho Holmium

67

167

Er Erbium

68

169

Tm Thulium

69

173

Yb Ytterbium

70

175

Lu Lutetium

71

Key

a

X b

a = relative atomic mass

X = atomic symbol

b = proton (atomic) number

232

Th Thorium

90

Pa Protactinium

91

238

U Uranium

92

Np Neptunium

93

Pu Plutonium

94

Am Americium

95

Cm Curium

96

Bk Berkelium

97

Cf Californium

98

Es Einsteinium

99

Fm Fermium

100

Md Mendelevium

101

No Nobelium

102

Lr Lawrencium

103

2


1 Bromine has a melting point of –2oC and a boiling point of 59

oC.

At which temperature is bromine a liquid?

2 At the same temperature and pressure, different gas molecules move with different

average speeds.

Which of the following lists the molecules in order of decreasing average speed?

fastest slowest

A ammonia methane chlorine sulphur dioxide

B ammonia methane sulphur dioxide chlorine

C methane ammonia sulphur dioxide chlorine

D methane ammonia chlorine sulphur dioxide

3 In an experiment, a student reacted ethanol with ethanoic acid to prepare ethyl

ethanoate. Which of the following procedure should he carry out to recover the ethyl

ethanoate from the reaction mixture?

A Add water and then separate by means of a separating funnel.

B Add water and carry out fractional distillation on the mixture.

C Filter and recover ethyl ethanoate on the filter paper.

D Carry out fractional distillation directly on the mixture.

4 The table shows the number of protons, neutrons and electrons in four ions.

For which ion is the data correct?

ion

number of

protons neutrons electrons

A 2

1H - 1 1 2

B 18

8 O 2- 10 8 12

C 40

20Ca 2+ 20 20 22

D 6 +

2 Li 3 3 2

-50 -25 0 25 50 75 100 125 150

A B C D


5 The proton umbers of elements, X, Y and Z are 4, 6 and 8 respectively. Which of the

following lists give the correct formulae of the compounds formed between them.

A X2Z YZ XYZ3

B XZ YZ2 XYZ3

C XZ YZ2 XYZ4

D X2Z YZ XYZ4

6 The table below shows some of the physical properties of some ‘unknown’ substances, P,

Q, R and S.

Unknown

substance

Melting

point / oC

Boiling

point /oC

Electrical conductivity Solubility in

water Solid state Liquid state

P 122 550 Poor Poor Insoluble

Q 690 1790 Poor Good Soluble

R 1510 2489 Poor Poor Insoluble

S 1453 2730 Good Good Insoluble

Which of the following statements about the four substances is correct?

A Substance P is a simple molecular compound with weak covalent bonds.

B Substance Q is an ionic compound with mobile electrons in the liquid state.

C Substance R is a macromolecule with immobile electrons held by strong

electrostatic forces.

D Substance S is a macromolecule with mobile electrons.

7 Which of the following equations best represents the reaction between hydrochloric acid

and sodium hydroxide?

A Na+ + Cl

- NaCl

B NaOH + H+ Na

+ + H2O

C HCl + OH- Cl

- + H2O

D H+ + OH

- H2O


8 The graph shows the pH of a sample of soil as lime (calcium oxide) is added.

How much lime has to be added to make the same sample of soil neutral?

A 1.5 g B 2.0 g

C 2.5 g D 3.0 g

9 Which statement is true of all acids in aqueous solution?

A They are used to acidify oxidising agents in redox reactions.

B They produce salt and water when reacted with metals.

C They are electrolytes because they are ionised in water.

D They turn methyl orange yellow when they neutralise an alkali.

10 Test on a sample of polluted water from a factory gave the following results.

reagent added result

nitric acid and aqueous barium nitrate white precipitate

aqueous ammonia white precipitate, insoluble in excess

Which compound could have been present in the water?

A zinc chloride B zinc sulphate

C aluminium chloride D aluminium sulphate


11 The flow diagram shows how precipitate M can be obtained from solid L.

What are L and M?

L M

A

B

C

D

CaCO3

CaCO3

Ca(OH)2

Ca(OH)2

CaCO3

Ca(OH)2

Ca(OH)2

CaCO3

12 Many properties of an element and its compounds can be predicted from the position

of the element in the Periodic Table.

What property could not be predicted in this way?

A its ability to conduct electricity

B its physical state

C its metallic or non-metallic properties

D the number of isotopes it has

13 Elements E, G and H belong to the same period in the Periodic Table. The properties

of the oxides of E, G and H are given in the table below.

Properties

Oxide of E Soluble in both hydrochloric acid and aqueous sodium hydroxide

Oxide of G Decolourises acidified aqueous potassium manganate(VII)

Oxide of H Insoluble in aqueous sodium hydroxide but soluble in dilute

hydrochloric acid

Which of the following gives the correct sequence of E, G and H in order of

increasing proton number in the Periodic Table?

A E, G, H B E, H, G

C H, E, G D G, E, H

white solid

L

colourless

gas

white solid colourless

solution

white precipitate

M

heat

water


14 Rubidium, Rb, is an alkaline metal. Which of the following properties is this metal likely

to have?

A soft, has low melting point, floats on water and reacts vigorously with water

B soft, has low melting point, sinks in water and reacts violently with water

C soft, has high melting point, floats on water and reacts vigorously with water

D soft, has high melting point, sinks in water and reacts violently with water

15 Melamine, a plastic, has the following composition by mass.

C: 28.6%, H: 4.80 %, N: 66.6%

If its relative molecular mass is 126, what is its molecular formula?

A CH2N2 B C2H4H4

C C3H6N6 D C4H8H8

16 All of the following substances produce carbon dioxide on complete combustion.

Which one will produce 1.0 mol of carbon dioxide?

A 0.25 mol of ethanol

B 0.5 mol of ethene

C 1.0 mol of propane

D 1.5 mol of graphite

17 When 250 cm3 of 3.00 mol/dm

3 hydrochloric acid is added to 350 cm

3 of 2.00 mol/dm

3

hydrochloric acid, the concentration of the solution of hydrochloric acid obtained in

mol/dm3 is

A 1.45 B 2.42

C 2.50 D 2.90


18 On adding aqueous lead(II) nitrate to aqueous potassium iodide, a precipitate is

immediately formed.

Pb2+

(aq) + 2I-(aq) PbI2(s)

A student decided to add various volumes of 1.0 mol/dm3 lead(II) nitrate to 5 cm

3 of 1.0

mol/dm3 aqueous potassium iodide. Each time, she centrifuged the mixture and measure

the height of the precipitate formed. Below are her results.

What volume of lead(II) nitrate did the student use in test-tube X to produce the maximum

height of the precipitate?

A 1.0 cm3 B 2.5 cm

3

C 5.0 cm3 D 10.0 cm

3

19 Which one of the following best describes what happens during the electrolysis of

concentrated sodium chloride solution between graphite electrodes?

A An unequal volume of gases is collected at the electrodes.

B The gaseous products dissolve in the solution to form hydrochloric acid.

C The pH of the solution remains constant.

D The sodium chloride solution becomes more diluted.

20 A solid deposit of element, R, is formed at the cathode when an aqueous solution

containing ions of R is electrolysed.

Which statement about element R must be correct?

A R ions gain electrons at the cathode.

B R gains electrons to form ions at the cathode.

C R is above hydrogen in the reactivity series.

D R ions diffuse faster than other ions to the cathode.

height of

precipitate

formed test-tube

X

Volume of lead(II) nitrate added / cm3


21 Three electrochemical cells are set up using copper metal and three unknown metals, U, V

and W as electrodes, immersed in dilute sulphuric acid of the same concentration.

The potential differences between the metals are given in the table below.

Electrochemical cell Metals used Voltage / V Positive electrode

1 Cu, U -0.45 U

2 Cu, V +1.11 Cu

3 Cu, W +2.71 Cu

From these results, deduce which of the following correctly list the metals in the order

of increasing ease of oxidation.

A U V Cu W

B W V Cu U

C U Cu V W

D W Cu V U

22 The heat-reflecting shields of some space rockets are gold-plated, using electrolysis.

Which electrodes and electrolyte would be used to gold-plate the heat shield?

Negative electrode Positive electrode Electrolyte

A

B

C

D

Carbon

Gold

Heat shield

Heat shield

Heat shield

Heat shield

Carbon

Gold

Gold compound

Copper compound

Copper compound

Gold compound

23 Which statement concerning energy change is false?

A

B

C

D

Heat energy is liberated when potassium reacts with water.

Light energy is absorbed during photosynthesis.

Light energy is produced when methane burns in oxygen.

Electrical energy is produced during electrolysis.


24 The rate of the reaction between a given mass of calcium carbonate and 1.0 mol/dm3

hydrochloric acid was studied by collecting the released carbon dioxide in a graduated

syringe. Some calcium carbonate was left behind.

The results are shown in the graph.

How would the results change if the experiment were repeated using the same mass of

calcium carbonate but half the volume of hydrochloric acid and of twice the

concentration?

Maximum volume of

carbon dioxide collected

Time at which the maximum

volume is first reached

A

B

C

D

45 cm3

45 cm3

90 cm3

90 cm3

less than 4 mins

more than 4 mins

less than 4 mins

more than 4 mins

25 In two separate experiments, manganese(IV) was added to 50 cm3 of aqueous hydrogen

peroxide. The measurements taken are shown in the table below.

experiment mass of

MnO2 / g

temperature

rise / oC

total volume of O2

produced / cm3

1

2

0.1

0.2

5.0

x

50

y

What were the values of x and y?

x y

A

B

C

D

5.0

10.0

20.0

20.0

50

50

50

100


26 Vanadium (V) oxide reacts with dilute sulphuric acid in their reaction shown below:

2 5 2 4 2 4 22V O + H SO VO SO + H O

In this reaction, vanadium (V) oxide is acting as a _______________.

A base B dehydrating agent

C oxidizing agent D reducing agent

27 In which one of the following reactions does the oxidation state of sulphur increase by

two?

A

B

C

D

SO32-

+ 2H+ SO2 + H2O

SO2 + Cl2 + 2H2O 4H+ + SO4

2- + 2Cl

-

S + O2 SO2

Zn + S ZnS

28 Dry ammonia gas was passed over heated copper(II) oxide.

In this reaction, the ammonia was __________________.

A decomposed B dehydrated

C reduced D oxidised

29 It was found that cars parked near beaches often corroded more quickly.

Which substance, when present in above average levels in the air, is a possible explanation

for this?

A carbon C salt

B oxides of nitrogen D sulphur dioxide


30 A sample of air was shaken with an alkaline solution of a compound called pyrograllol.

The gases remaining did not support combustion.

Which one of the following pairs of gases was removed from the air by the alkaline

pyrograllol?

A oxygen and nitrogen

B oxygen and carbon dioxide

C oxygen and water vapour

D carbon dioxide and nitrogen

31 Ammonium chloride may be used to prepare ammonia by heating it with ________.

A water.

B dilute nitric acid.

C aqueous sodium nitrate.

D aqueous sodium hydroxide.

32 In the Haber process for the manufacture of ammonia, what are the usual operating

conditions?

Pressure / atm Temperature / oC Catalyst

A

B

C

D

250

250

250

250

450

450

450

450

Iron

Iron(III) oxide

vanadium

vanadium(V) oxide

33 Why does aluminium have an apparent lack of reactivity?

A Aluminium is low in the reactivity series.

B Aluminium has triple bonds that are hard to break.

C Aluminium has a coating of aluminium oxide, preventing further reaction

D Aluminium has a high melting point and requires a lot of energy for reaction.


34 The diagram shows the apparatus used in an experiment to reduce substance Q with

the gas generated n the conical flask.

Which one of the following pairs could be P and Q?

P Q

A lead copper(II) oxide

B copper lead(II) oxide

C zinc magnesium oxide

D magnesium iron(III) oxide

35 Solder is an alloy of lead and tin. Which property is true of solder and makes it useful

for joining metals together?

A It is less dense than its pure metals.

B It is stronger than its constituent metals.

C It is less likely to corrode than its constituent metals.

D It has a lower melting point than its pure metals.


36 The diagram (figure 7) shows the fractional distillation of petroleum.

Which statements about fractions X and Y are correct?

X burns more

easily than Y

X has a lower boiling

point than Y

A

B

C

D

Yes

Yes

No

No

No

Yes

No

Yes

37 Useful fractions are obtained by the fractional distillation of petroleum oil. Which fraction

and use are correct?

fraction use

A bitumen fuel in cars

B petrol (gasoline) aircraft fuel

C paraffin (kerosene) for making roads

D lubricating fraction for making waxes and polishes

38 A molecule of hydrocarbon C16H34 undergoes cracking to produce a molecule of butane

and a number of ethene molecules. How many ethene molecules are produced?

A one B four

C six D twelve

heated

petroleum

Fraction X

FractionY

Figure 7


39 The molecular formula of oleic acid is C18H32O2.

How many double bonds between carbon atoms are present in one molecule of oleic acid?

A 1 B 2

C 3 D 4

40 Which pair of structures are isomers of each other?

A

B

C

D

C C

H

H

H

H

H

H

C C

H

H

H

H

C

H

H

H

H

C C

H

H

H

O

O H

C C

H

H

H

H

O

H

H

C C

H

H

H

H

C

H

H

O

H

H

C C

H

H

H

O

C

H

H

H

H

H

C C

H

HH

H

C C

H

H

H

H

C

H

H

C

H

H

H

H

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